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For the react...

Question

For the reaction $H_{2} + I_{2} ⇌ 2 H I$ :

A

K_{c} = 2 K_{p}

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B

K_{c} > K_{p}

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C

K_{c} = K_{p}

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D

K_{c} < K_{p}

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Solution

The correct option is D $K_{c} = K_{p}$
As we know,
$K_{p} = K_{c} {(R T)}^{Δ n}$
For reaction:
$H_{2} + I_{2} ⇌ 2 H I$
$Δ n = 0 s o K_{p} = K_{c}$

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Similar questions

Q. Assertion :For the reaction

H_{2} + I_{2} ⇌ 2 H I, K_{p} = K_{c}

K_{p} = K_{C}

for a reaction, the sum of stoichiometric coefficient of reactants should be equal to the sum of stoichiometric coefficients of products.

The relation between equilibrium constant $K_{P}$ and $K_{C}$ is

K_{p} = K_{c}

for all reactions. BECAUSE Reason:

K_{p}

K_{c}

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K_{p} = K_{c} {(R T)}^{Δ n}

.

Q. For the reaction,

2 N O_{2} (g) ⇌ 2 N O (g) + O_{2} (g)

K_{c} = 1.8 \times 10^{- 6}

184^{o} C

(R = 0.0831 k J / (m o l . K J))

K_{p}

K_{c}

are compared at

184^{o} C

it is found that
(1) Whether

K_{p}

is greater then, less then or equal to

K_{c}

depends upon the total gas pressure
(2)

K_{p} = K_{c}

K_{p}

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K_{p}

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For a general reaction aA(g) + bB(g) $⇋$ cC(g)+ dD(g), what is the relationship between the equilibrium constants $K_{c}$ and $K_{p}$ ? [assume $Δ$ n = $μ$ = (c + d) - (a+b) ]\)

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